Ch.7 - Quantum MechanicsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Before quantum mechanics was developed, Johannes Rydberg developed an equation that predicted the wavelengths (λlambda) in the atomic spectrum of hydrogen: 1/λ = R(1/m2 - 1/n2). In this equation R is

Solution: Before quantum mechanics was developed, Johannes Rydberg developed an equation that predicted the wavelengths (λlambda) in the atomic spectrum of hydrogen: 1/λ = R(1/m2 - 1/n2). In this equation R is

Problem

Before quantum mechanics was developed, Johannes Rydberg developed an equation that predicted the wavelengths (λ) in the atomic spectrum of hydrogen: 1/λ = R(1/m2 - 1/n2). In this equation R is a constant and m and n are integers. Use the quantum-mechanical model for the hydrogen atom to derive the Rydberg equation.

Solution
  • For an H atom, the energy of an electron in level n is represented as:

  • An electron jumping from higher energy level f to lower energy level i, the energy released by atom will appear as:

  • Use the equation of En to find the ΔE.

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